According to the outline, you need to understand how the collision model accounts for the temperature dependence of reactions. So in collision theory, molecules must collide at a minimum kinetic energy in order to break bonds and form new ones. The higher the temperature, the higher the kinetic energy of the molecules.

As long as you understand that collision is necessary for reactions to continue, molecules need to break apart and form and with and increase in temperature this will happen more I think you should be okay.

Based off of what we went over in lecture, know that at higher temperatures, there are more collisions and that reactants must collide with enough energy to break bounds, thus overcoming the activation energy barrier. Furthermore, reactants must have the correct orientation when they collide (frequency factor A).

For reactions to occur, collisions btwn reactants must occur. The # of reactants in the elementary step gives us the molecularity and thus the order. Also, these collisions must occur at a correct orientation, which is why we use frequency factor A (a constant) in the Arrhenius equation.

kevinolvera1j wrote:You should probably know that collisions need to have the appropriate amount of energy to break a bond and also be correctly oriented in order for a new molecule to form.

This is also why we only cover up to second-order reactions, since it's much more difficult to get 3 or more molecules to all collide at the same time with the right amount of energy and the correct orientation.

Collision theory connects temperature and energy. Molecules need to have enough kinetic energy that, upon collision, there is enough energy to overcome the energy barrier. By increasing temperature, the molecules have a higher kinetic energy and therefore are more likely to overcome the energy barrier, increasing the rate of the reaction.